An H₂/H⁺ half-cell (anode) and an Ag⁺/Ag half cell (cathode) are connected by a wire and a salt bridge. (a) Sketch the cell, indicating the direction of electron and ion flow.

Key Concepts

Electrochemical Cells

Electrochemical cells consist of two half-cells, where oxidation occurs at the anode and reduction at the cathode. In this setup, the H2/H+ half-cell serves as the anode, where hydrogen gas is oxidized to protons, while the Ag+/Ag half-cell acts as the cathode, where silver ions are reduced to solid silver. Understanding the flow of electrons and ions is crucial for analyzing the cell's operation.

Electron Flow

In an electrochemical cell, electrons flow from the anode to the cathode through an external circuit. This flow occurs because oxidation at the anode generates electrons, which are then attracted to the cathode, where reduction takes place. Recognizing the direction of electron flow is essential for understanding how the cell generates electrical energy.

Salt Bridge Function

A salt bridge is a crucial component of an electrochemical cell that maintains electrical neutrality by allowing the flow of ions between the two half-cells. It typically contains a gel or solution of an inert electrolyte, which helps balance the charge as electrons move through the external circuit. Understanding the role of the salt bridge is important for ensuring the continuous operation of the cell.